If Delta U and Delta W represent increase in internal energy and work done by system respectively in

English

Gujarati

Hindi

11.Thermodynamics

normal

If $\Delta U$ and $\Delta W$ represent the increase in internal energy and work done by the system respectively in a thermodynamic process, which of the following is true?

A

$\Delta U = -\Delta W$ , in a isothermal process

B

$\Delta U = -\Delta W$ ,in a adiabatic process

C

$\Delta U = \Delta W$ , in a isothermal process

D

$\Delta U = \Delta W$ ,in a adiabatic process

Solution

In adiabatic process $Q=0$

$\mathrm{Q}=\mathrm{W}+\Delta \mathrm{U}$

$\Delta \mathrm{U}=-\mathrm{W}$

Standard 11

Physics

Share

Similar Questions

$1\;g$ of water, of volume $1\; \mathrm{cm}^{3}$ at $100^{\circ} \mathrm{C},$ is converted into steam at same temperature under normal atmospheric pressure $\left(=1 \times 10^{5} \;\mathrm{Pa}\right) .$ The volume of steam formed equals $1671 \;\mathrm{cm}^{3} .$ If the specific latent heat of vaporisation of water is $2256\; \mathrm{J} / \mathrm{g}$, the change in intemal energy is…..$J$

normal

Pressure-temperature relationship for an ideal gas undergoing adiabatic change is $\left( {\gamma = {C_p}/{C_v}} \right)$

normal

For free expansion of a gas, which is true

normal

Six moles of an ideal gas perfoms cycle shown in figure. If the temperature $T_A = 600\, K$, $T_B = 800\, K, T_C = 2200\, K$ and $T_D = 1200\, K$, the work done per cycle is…….. $kJ$

normal

$2$ moles of a diatomic gas undergoes the process : $PT_2/V$ = constant. Then, the molar heat capacity of the gas during the process will be equal to

normal